Using the balanced equation Mg(s)+2HCl(aq)>MgCl2(aq)+H2(g), what volume of hydrogen would be produced by the reaction of...

Using the balanced equation Mg(s)+2HCl(aq)>MgCl2(aq)+H2(g), what volume of hydrogen would be produced by the reaction of 2.00 g of magnesium with an excess of hydrochloric acid at 746 torr and 26.2°C?

Expert Solution

queen_honey_blossom answered 2 years ago

The reaction is: Mg(s) + 2HCl(aq) --> MgCl2 (aq) + H2(g) 1. If 2.016 g of...

The reaction is: Mg(s) + 2HCl(aq) --> MgCl2 (aq) + H2(g) 1. If 2.016 g of hydrogen (H2) was released, how many moles of magnesium reacted? How many grams of magnesium would this be? 2. How many moles of magnesium would replace one mole of hydrogen (H) in the hydrochloric acid? How many grams? (This is the equivalent weight) 3. Compare the mass calculated above in question 2 to your experimental equivalent weight and calculate the percent difference. What would...

Mg metal reacts with HCl to produce hydrogen gas. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g)......A)What volume of hydrogen at 0 ∘C...

Mg metal reacts with HCl to produce hydrogen gas. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g)......A)What volume of hydrogen at 0 ∘C and 1.00 atm (STP) is released when 9.25 g of Mg reacts B)How many grams of magnesium are needed to prepare 3.90 L of H2 at 730 mmHg and 20 ∘C

Given : 2HCl(aq) + Mg(s) -> MgCl2(aq) +H2(g) Mg(s) + 1/2 O2(g) -> MgO(s) Mass of...

Given : 2HCl(aq) + Mg(s) -> MgCl2(aq) +H2(g) Mg(s) + 1/2 O2(g) -> MgO(s) Mass of 3.00M HCl (diluted in water) : 88.4g Vol of 3.00M HCl : 87.5mL Mass of Mg : 0.599g Total mass: 88.999g --------------------------------------------------------------------------------------- Find mole of product IF: (show calculations) A. HCl is the limiting reactant: ______ B. Mg is the limiting reactant: ______

Reaction of HCl (aq) and Mg(s) to form MgCl2(aq) and H2(g) Given: Molarity of HCL :...

Reaction of HCl (aq) and Mg(s) to form MgCl2(aq) and H2(g) Given: Molarity of HCL : 3.00M volume of HCL: 20.0mL mass of Mg: 0.036g volume of gas before placing in equalization chamber: 37.0mL volume of gas after placing in equalization chamber: 37.5 mL barometric pressure of the room: 736.4 mmhg temperature of the room: 18.5 C ------------------------------------------------ Calculate: mole of Mg reacted: mole of H2(g) formed: vapor pressure of vater: pressure of H2 (Daltons Law): pressure of H2 in...

Mg(s)+2HCl(aq)=MgCl2(aq)+H2(g) (A) 0.0675g Mg AND 4mL of 6M HCl were used. Barometric pressure were 28.85 inches...

Mg(s)+2HCl(aq)=MgCl2(aq)+H2(g) (A) 0.0675g Mg AND 4mL of 6M HCl were used. Barometric pressure were 28.85 inches Hg. A volume of 73.6mL of hydrogen was collected at a temperature of 26.0C. The vapor pressure of water is 25.2mm Hg at this temperature. Calculate R, the gas law constant, in L-atom\mol-K using the information above for the reaction of HCl and Mg. 760 mmHg= 1.00atm. 1 inch=2.54 cm. Show your calculation (B) why is it necessary to substract the vapor pressure of...

Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.107 g...

Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.107 g of Zn(s) is combined with enough HCl to make 54.9 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.0 ∘C to 24.0 ∘C. Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g⋅∘C as the specific heat capacity.)

A. In the experiment, The molar volume of a gas. Mg (s) + 2HCl (aq) =...

A. In the experiment, The molar volume of a gas. Mg (s) + 2HCl (aq) = MgCl2 (aq) + H2 (g), the magnesium ribbon was dissolved in hydrochloric acid, a monoprotic acid, to produce H2 gas. If phosphoric acic, a triprotic acid, were used to react with the magnesium rather than hydrochloric acid, does that affect the amount of H2 gas produced?. Write balanced equations for the reaction og Mg with 1) HCl and 2) phosphoric acid to help explain...

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) How many...

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) How many liters of H2 would be formed at 636 mm Hg and 17 ∘C if 27.0 g of zinc was allowed to react? How many grams of zinc would you start with if you wanted to prepare 6.85 L of H2 at 284 mm Hg and 28.5 ∘C?

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl : Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) 1)How...

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl : Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) 1)How many liters of H2 would be formed at 592 mm Hg and 17 ∘C if 25.5 g of zinc was allowed to react? 2)How many grams of zinc would you start with if you wanted to prepare 4.60 L of H2 at 294 mm Hg and 34.5 ∘C ?

Consider the reaction Fe(s) + 2HCl(aq)FeCl2(s) + H2(g) for which H° = -7.400 kJ and S°...

Consider the reaction Fe(s) + 2HCl(aq)FeCl2(s) + H2(g) for which H° = -7.400 kJ and S° = 107.9 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.097 moles of Fe(s) react under standard conditions at 298.15 K. Suniverse = J/K (2) Is this reaction reactant or product favored under standard conditions? _________reactantproduct (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is...

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